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INORGANIC & ORGANIC CHEMISTRY > Matter and Measurement > Flashcards

Matter and Measurement Flashcards

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1
Q

is the field of study concerned with the characteristics, composition, and transformations of matter

A

Chemistry

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2
Q

includes all things, both living and non-living.

A

Matter

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3
Q

Physical state

A

Solid
Liquid
Gas

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4
Q

characterized by a definite shape and a definite volume

A

Solid

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5
Q

characterized by an indefinite shape and a define volume

A

Liquid

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6
Q

characterized by an indefinite shape and an indefinite volume

A

Gas

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7
Q

distinguishing characteristic of a substance that is used in its identification and description

A

Property

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8
Q

characteristics that can be observed without changing the basic identity of the substance (ex. Color, odor, physical state, melting/boiling point, hardness)

A

Physical property

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9
Q

describes the way the substance undergoes or resists change to form a new substance

A

Chemical property

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10
Q

a substance changes its physical appearance but not is chemical composition (ex. Changes in physical state)

A

Physical change

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11
Q

a substance undergoes a change in chemical composition. It always involve conversion of the material under consideration into one or more new substances

A

Chemical change

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12
Q

a single kind of matter that cannot be separated into other kinds of matter by any physical means

A

Pure substance

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13
Q

-physical combination of two or more pure substances in which each substance retains its own chemical identity
-One characteristic of any mixture is that its components can be separated using physical means

A

Mixture

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14
Q

a mixture that contains visible different phases (parts), each of which has different property

A

Heterogenous mixture

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15
Q

contains only one visibly distinct phase (part), which has a uniform properties throughout (ex. Sugar-water mixture)

A

Homogenous mixture

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16
Q

pure substance that cannot be broken down into simpler pure substances by chemical means

A

Element

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17
Q

pure substance that can broken down into two or more simpler pure substances by chemical means (ex. Water [H2O] can be broken down into the elements hydrogen and oxygen)

A

Compound

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18
Q

Notes: Compounds vs Mixtures
-Remember, substances can be combined either physically or chemically
-No such binding occurs during physical combination

A

Notes:
-Physical combination of substances produces a mixture
-Chemical combination of substances produces a compound, a substance in which combining entities are bound together

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19
Q

The discovery and isolation of the 117 known elements, the building blocks for all matter, have taken place over a period of several centuries. Most of the discoveries have occurred since

A

1700, the 1800s being the most active period

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20
Q

Note: Elements
Each element has a unique name; some bear geographical names (germanium, francium and polonium), some are named for the planets (mercury, uranium, neptunium), some reflect specific properties of the element or of the compounds containing it

A
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21
Q

one- or two-letter designation for an element derived from the elementโ€™s name

A

Chemical symbol

22
Q

is the smallest particle of an element that can exist and still have the properties of the element

A

Atom

23
Q

Note:
-A sample of any element is composed of atoms of a single type, those of that element. In contrast, a compound must have two or more types of atoms present, because by definition at least two elements must be present
-Free atoms are rarely encountered in nature
-Atoms are almost always found together in aggregates or clusters

A
24
Q

is a group of two or more atoms that functions a unit because the atoms are tightly bound together

A

Molecules

25
Q

is a molecule that contains two atoms, a triatomic molecule contains three, and so on.

A

diatomic molecule

26
Q

is a molecule in which all atoms present are of the same kind. Substances containing (ex. Hydrogen [H2], oxygen [O2], nitrogen [N2], and chlorine [Cl2])

A

homoatomic molecule

27
Q

is a molecule in which two or more kinds of atoms are present.

A

heteroatomic molecule

28
Q

Note:
-The atoms present may all be of the same kind, or two or more kinds may be present
-Substances containing heteroatomic molecules are compounds (ex. Water [H2O]

A
29
Q

molecules made of atoms from different elements

A

Compounds

30
Q

atoms connected by chemical bond

A

Molecules

31
Q

Note:
ALL COMPOUNDS ARE MOLECULES, BUT NOT ALL MOLECULES ARE COMPOUNDS
H2 is a molecule, but not a compound (only H is present)
H2O is both a molecule and a compound (H and O are present)

A
32
Q

is a notation made up of the chemical symbols of the elements present in a compound and numerical subscripts (located to the right of each chemical symbol) that indicate the number of atoms of each element present in a molecule of the compound.

A

chemical formula

33
Q

determination of the dimensions, capacity, quantity, or extent of something

A

Measurement

34
Q

Note:
There are two systems of measurement that is used commonly: The English system of units and the metric system of units

A
35
Q

Examples of units in the English system are

A

inch, foot, pound, quart, and gallon

36
Q

Examples of units in the metric system are

A

gram, meter, and liter

37
Q

Examples of units in the metric system are

A

gram, meter, and liter

38
Q

Note: Metric System Units
-In the metric system, there is one base unit for each type of measurement
-Prefixes are then added to the base unit
-The meter (m) is the base unit of length in the metric system (1 m is equivalent to 1.09 yards)
-The gram (g) is the base unit of mass in the metric system (28 g = 1 ounce, 454 g = 1 pound)
-The liter (L) is the base unit of volume in the metric system (1 L is equivalent to 1.06 quarts)

A
39
Q

Measurements will always have a degree of uncertainty or error

A

Uncertainty in Measurements

40
Q

are digits in a measurement that are known with certainty plus one digit that is estimated

A

Significant figures

41
Q

are digits in a measurement that are known with certainty plus one digit that is estimated

A

Significant figures

42
Q

note:
-Uncertainty is indicated by the number of significant figures recorded
-Number of significant figures = all certain digits + one estimated digit

A
43
Q

. In multiplication and division, the number of significant figures

A

that contains the fewest significant figures

44
Q

In addition and subtraction, the answer is given with as many significant figures as the measurement with the

A

least number of decimal places

45
Q

is a numerical system in which numbers are expressed in the form A X 10n, where A is a number with a single nonzero digit to the left of the decimal place and n is a whole number

A

Scientific notation

46
Q

Note:
-The coefficients are combined in the usual way (multiplied or divided)
-The rules for exponential terms are:
1. To multiply exponential terms, add the exponents
2. To divide the exponential terms, subtract the exponents
Ex. (2.33 x 103) x (1.55 x 104)
2.33 x 1.55 = 3.61
103 x 104 = 103+4 = 107
Final answer is 3.61 x 107

A
47
Q

is a ratio that specifies how one unit of measurement is related to another unit of measurement
It is derived from equalities that relate units
Ex. 1 minute = 60 seconds
A pair of conversion factor can be derived from this equality
(1 ๐‘š๐‘–๐‘›๐‘ข๐‘ก๐‘’)/(60 ๐‘ ๐‘’๐‘๐‘œ๐‘›๐‘‘๐‘ ) and (60 ๐‘ ๐‘’๐‘๐‘œ๐‘›๐‘‘๐‘ )/(1 ๐‘š๐‘–๐‘›๐‘ข๐‘ก๐‘’)

A

Conversion Factors

48
Q

is a general problem-solving method in which the units associated with numbers are used as a guide in setting up calculations

A

Dimensional Analysis

49
Q

-is the ratio of the mass of an object to the volume occupied by that object
-Generally expressed in grams per cubic centimeter (g/cm3) for solids, grams per milliliters (g/mL) for liquids

A

๐‘ซ๐’†๐’๐’”๐’Š๐’•๐’š

50
Q

๐‘ซ๐’†๐’๐’”๐’Š๐’•๐’š formula

A

๐‘ซ๐’†๐’๐’”๐’Š๐’•๐’š= ๐’Ž๐’‚๐’”๐’”/๐’—๐’๐’๐’–๐’Ž๐’†

51
Q

is a form of energy. Temperature is an indicator of the tendency of heat energy to be transferred

A

Heat

52
Q

Note:
-Heat energy flows from objects of higher temperature to objects of lower temperature.
-Both the Celsius and the Kelvin are part of the metric system; Fahrenheit scale belongs to the English system
-The Celsius scale is the most commonly used in scientific work

A

INORGANIC & ORGANIC CHEMISTRY (7 decks)

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